but that last part is really [tex]2H_2O[/tex]. But if i write it like that, then in my net equation i gotta keep [tex]H_2O[/tex] and the H and OH ... making my net equation the same as my ionic equation. That seems wrong to me. Is there a covention where I can write [tex]2H_2O[/tex] and still leave out OH and H as spectator ions in my net ionic equation? Thank you for your time.

First check if [itex]Mg(ClO_4)_2[/itex] is a solid, otherwise it would remain hydrated and would not appear in the net ionic equation. And I believe that water will actually be in the net ionic equation, that is [itex]H^+_{(aq)} + OH^-_{(aq)} \xrightarrow{\leftarrow} H_2O_{(l)}[/itex], there's a equilibrium associated with this equation although not on a large scale.

ERROR - yeah that mg clo4 is solid, it has (s) in subscript beside it.
EDIT - whoops. That was my assumption. If HCLO is breaking it down, then it'd have to be a liquid, as this kind of reaction goes to completion.

First, think about it.......how is bromine gas even formed? You've got two anions, the two cannot combine unless one of them is a cation. So bromine anion is the final product, usually the ammonium cation interacts ionically with bromine anion to a degree to form a salt adduct (l). However, I don't believe that you need to get this technical here. Thus your net ionic equation seems correct.